http://www.anarchistcookbook.com/member.php?u=6140 A social site powered by it's members en H.Atakan KOC www.sonkonu.com 60 http://www.anarchistcookbook.com/showthread.php?t=6377 Mon, 09 Jul 2007 23:18:57 GMT Anyone who is living in holland could help.]]> http://www.anarchistcookbook.com/showthread.php?t=6377 Bullshit firetime27> http://www.anarchistcookbook.com/showthread.php?t=5097 Mon, 05 Mar 2007 23:55:27 GMT In a 2000 mL beaker pour 1900 mL of bleach and place in the ice bath and cool to about 0*C.
Add 95mL of acetone. And stir it in don't let the temp exceed 50*C.
Let the chloroform settle to the bottom and collect it and discard the rest of the liquid. Yield is crappy but deal with it your chems are sheap as hell.
Distill the chloroform if you want a decent product.]]> http://www.anarchistcookbook.com/showthread.php?t=5097 Pyro firetime27> http://www.anarchistcookbook.com/showthread.php?t=5096 Mon, 05 Mar 2007 23:51:39 GMT
The mole (symbol: mol) is the SI base unit that measures an amount of substance. One mole contains Avogadro's number (approximately 6.022×1023) entities. A mole is much like "a dozen" in that both units can describe any set of elementary objects, although the mole's use is usually limited to measurement of subatomic, atomic, and molecular structures. This is all due to the fact that a mole represents an exceedingly large number of entities.

Utility of moles

The mole is useful in chemistry because it allows different substances to be measured in a comparable way. Using the same number of moles of two substances, both amounts have the same number of molecules or atoms. The mole makes it easier to interpret chemical equations in practical terms. Thus the equation:

2H2 + O2 → 2H2O

can be understood as "two moles of hydrogen plus one mole of oxygen yields two moles of water."

Moles are useful in chemical calculations, because they enable the calculation of yields and other values when dealing with particles of different mass.

Number of particles is a more useful unit in chemistry than mass or weight, because reactions take place between atoms (for example, two hydrogen atoms and one oxygen atom make one molecule of water) that have very different weights (one oxygen atom weighs almost 16 times as much as a hydrogen atom). However, the raw numbers of atoms in a reaction are not convenient, because they are very large; for example, just one mL of water contains over 3×1022 (or 30,000,000,000,000,000,000,000) molecules.

[edit] Example calculation

In this example, moles are used to calculate the mass of CO2 given off when 1 g of ethane is burned. The equation for this chemical reaction is:

7 O2 + 2 C2H6 → 4 CO2 + 6 H2O

that is,

7 molecules of oxygen react with 2 molecules of ethane to give 4 molecules of carbon dioxide and 6 molecules of water.

The first thing is to figure out how many molecules of ethane were burnt. We know that it was just enough to make 1 g, so we now need the molecular mass of ethane. This can be calculated : the mass in grams of one mole of a substance is by definition its atomic or molecular mass; The atomic mass of hydrogen is 1, and the atomic mass of carbon is 12, so the molecular mass of C2H6 is (2 × 12) + (6 × 1) = 30. One mole of ethane is 30 g. So 1 g of ethane is 1/30th of a mole; the amount burnt was 1/30th of a mole (remember that it is a number, quite like "half a dozen").

Now we can calculate the number of molecules of CO2 given off. Since for 2 molecules of ethane we obtain 4 molecules of CO2, we have 2 molecules of CO2 for each molecule of ethane. So, for 1/30th of a mole of ethane, 2 × 1/30th = 1/15th of a mole of CO2 were produced.

Next, we need the molecular mass of CO2. The atomic mass of carbon is 12 and that of oxygen is 16, so one mole of carbon dioxide is 12 + (2 × 16) = 44 g/mol.

Finally, the mass of CO2 is 1/15 mol × 44 g/mol = 2.93 g of carbon dioxide.

Notice that the number of moles does not need to balance on either side of the equation. This is because a mole does not count mass or the number of atoms involved, but the number of particles involved (each of them composed of a variable number of atoms). However, we could likewise calculate the mass of oxygen consumed, and the mass of water produced, and observe that the mass of products (carbon dioxide and water) is equal to the mass of dioxygen plus ethane:

* (7/2)(1/30th mol of dioxygen) (2 × 16 g/mol) = 7×16/30 g = 3.73 g
* (6/2)(1/30th mol of water)(2×1 + 16 g/mol) = 1.8 g
* 3.73 g + 1 g = 2.93 + 1.8 g

(Note: According to the mass-energy relationship, there is a very small difference between the mass of carbon, hydrogen and oxygen separated, on one side, and on the other side the mass of the molecules made of them; this has not been accounted for here.)

NOW GET TO WORK.]]> http://www.anarchistcookbook.com/showthread.php?t=5096 Pyro firetime27> http://www.anarchistcookbook.com/showthread.php?t=4767 Sun, 11 Feb 2007 01:30:22 GMT
http://www.apcforum.net/forums/

http://www.roguesci.org/megalomania/explosives.html

https://sciencemadness.org/talk/

http://www.thechemicalshop.com/

http://www.xsorbit2.com/users/apcfor...igh_Explosives

http://www.researchsupply.net/home.html

http://www.brainerdchemical.com/Brai...OVMTC=advanced]]> http://www.anarchistcookbook.com/showthread.php?t=4767 Pyro firetime27> http://www.anarchistcookbook.com/showthread.php?t=4425 Wed, 31 Jan 2007 22:42:51 GMT http://www.anarchistcookbook.com/showthread.php?t=4425 Pyro firetime27> http://www.anarchistcookbook.com/showthread.php?t=4062 Sat, 06 Jan 2007 03:51:27 GMT http://www.anarchistcookbook.com/showthread.php?t=4062 Drugs General Discussion firetime27> http://www.anarchistcookbook.com/showthread.php?t=3802 Mon, 04 Dec 2006 23:45:56 GMT http://www.anarchistcookbook.com/showthread.php?t=3802 Pyro firetime27> http://www.anarchistcookbook.com/showthread.php?t=2909 Mon, 28 Aug 2006 01:40:18 GMT http://www.ebaumsworld.com/whaleblowup.html

I guess thats one way to take care of it.]]> http://www.anarchistcookbook.com/showthread.php?t=2909 Pyro firetime27> http://www.anarchistcookbook.com/showthread.php?t=2886 Thu, 24 Aug 2006 07:02:08 GMT http://www.anarchistcookbook.com/showthread.php?t=2886 Pyro firetime27> http://www.anarchistcookbook.com/showthread.php?t=2885 Thu, 24 Aug 2006 05:40:24 GMT http://www.anarchistcookbook.com/showthread.php?t=2885 Pyro firetime27> http://www.anarchistcookbook.com/showthread.php?t=2878 Wed, 23 Aug 2006 06:02:55 GMT http://www.anarchistcookbook.com/showthread.php?t=2878 Pyro firetime27> http://www.anarchistcookbook.com/showthread.php?t=2876 Wed, 23 Aug 2006 02:47:17 GMT http://www.anarchistcookbook.com/showthread.php?t=2876 Pyro firetime27> http://www.anarchistcookbook.com/showthread.php?t=2873 Tue, 22 Aug 2006 20:49:17 GMT
http://www.roguesci.org/megalomania/explosives.html]]> http://www.anarchistcookbook.com/showthread.php?t=2873 Pyro firetime27> http://www.anarchistcookbook.com/showthread.php?t=2872 Tue, 22 Aug 2006 20:31:41 GMT http://www.anarchistcookbook.com/showthread.php?t=2872 Pyro firetime27> http://www.anarchistcookbook.com/showthread.php?t=2852 Sun, 20 Aug 2006 00:57:49 GMT http://www.anarchistcookbook.com/showthread.php?t=2852 Pyro firetime27> http://www.anarchistcookbook.com/showthread.php?t=2833 Wed, 16 Aug 2006 07:34:43 GMT http://www.anarchistcookbook.com/showthread.php?t=2833 Pyro firetime27> http://www.anarchistcookbook.com/showthread.php?t=2599 Sat, 15 Jul 2006 03:15:11 GMT
http://i87.photobucket.com/albums/k1...x/CO2laser.gif]]> http://www.anarchistcookbook.com/showthread.php?t=2599 Pyro firetime27> http://www.anarchistcookbook.com/showthread.php?t=2522 Fri, 07 Jul 2006 20:07:19 GMT http://www.anarchistcookbook.com/showthread.php?t=2522 Pyro firetime27> http://www.anarchistcookbook.com/showthread.php?t=1923 Thu, 04 May 2006 02:04:34 GMT
To extract DXM from robotussin convert the DXM to a free base with a strong base. Then dissolve the free base in a nonpolar solvent. Then extract with an acid and evaporate to collect the DXM]]> http://www.anarchistcookbook.com/showthread.php?t=1923 Drugs General Discussion firetime27>